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Related Concept Videos

Colors and Magnetism03:02

Colors and Magnetism

Color in Coordination Complexes
When atoms or molecules absorb light at the proper frequency, their electrons are excited to higher-energy orbitals. For many main group atoms and molecules, the absorbed photons are in the ultraviolet range of the electromagnetic spectrum, which cannot be detected by the human eye. For coordination compounds, the energy difference between the d orbitals often allows photons in the visible range to be absorbed and emitted, which is seen as colors by the human eye.
EDTA: Auxiliary Complexing Reagents01:26

EDTA: Auxiliary Complexing Reagents

EDTA titrations are usually carried out in highly basic conditions, where the fully deprotonated form of EDTA, Y4−, actively complexes with the free metal ions in the solution. Several metal ions precipitate as hydrous oxide (hydroxides, oxides, or oxyhydroxides) under these conditions, lowering the concentration of free metal ions in the solution. For this reason, auxiliary complexing agents or ligands such as ammonia, tartrate, citrate, or triethanolamine are used in EDTA titrations to...
EDTA: Chemistry and Properties01:22

EDTA: Chemistry and Properties

Polydentate ligands are most widely used in complexometric titrations because they form more stable complexes with the metal ions than mono- or bidentate ligands due to the chelate effect. Examples of polydentate ligands are ethylenediaminetetraacetic acid (EDTA), crown ethers, and cryptands. The most important feature of optimal polydentate ligands is the ability to form 1:1 complexes in a single-step process. Amino carboxylic acid derivatives are frequently used as complexing agents. EDTA is...
Crystal Field Theory - Tetrahedral and Square Planar Complexes02:46

Crystal Field Theory - Tetrahedral and Square Planar Complexes

Tetrahedral Complexes
Crystal field theory (CFT) is applicable to molecules in geometries other than octahedral. In octahedral complexes, the lobes of the dx2−y2 and dz2 orbitals point directly at the ligands. For tetrahedral complexes, the d orbitals remain in place, but with only four ligands located between the axes. None of the orbitals points directly at the tetrahedral ligands. However, the dx2−y2 and dz2 orbitals (along the Cartesian axes) overlap with the ligands less than the dxy,...
Ions as Acids and Bases02:54

Ions as Acids and Bases

Salts with Acidic Ions
Salts are ionic compounds composed of cations and anions, either of which may be capable of undergoing an acid or base ionization reaction with water. Aqueous salt solutions, therefore, may be acidic, basic, or neutral, depending on the relative acid-base strengths of the salt’s constituent ions. For example, dissolving the ammonium chloride in water results in its dissociation, as described by the equation:
Ionic Crystal Structures02:42

Ionic Crystal Structures

Ionic crystals consist of two or more different kinds of ions that usually have different sizes. The packing of these ions into a crystal structure is more complex than the packing of metal atoms that are the same size.
Most monatomic ions behave as charged spheres, and their attraction for ions of opposite charge is the same in every direction. Consequently, stable structures for ionic compounds result (1) when ions of one charge are surrounded by as many ions as possible of the opposite...

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Related Experiment Video

Updated: Jun 5, 2026

Thermochemical Studies of Ni(II) and Zn(II) Ternary Complexes Using Ion Mobility-Mass Spectrometry
16:11

Thermochemical Studies of Ni(II) and Zn(II) Ternary Complexes Using Ion Mobility-Mass Spectrometry

Published on: June 8, 2022

Hexaaqua-zinc(II) dipicrate.

S Natarajan, K V Vijitha, S A Martin Britto Dhas

    Acta Crystallographica. Section E, Structure Reports Online
    |January 5, 2011
    PubMed
    Summary

    This study details the crystal structure of a zinc(II) compound with picrate anions. The zinc ion exhibits octahedral coordination with water molecules, and the structure is stabilized by hydrogen bonds.

    Area of Science:

    • Inorganic Chemistry
    • Crystallography
    • Coordination Chemistry

    Background:

    • Zinc(II) complexes are widely studied for their diverse coordination geometries and potential applications.
    • Picrate anions are known for their energetic properties and ability to form crystalline salts.

    Purpose of the Study:

    • To elucidate the crystal structure and coordination environment of a novel zinc(II)-picrate compound.
    • To investigate the intermolecular interactions, specifically hydrogen bonding, within the crystal lattice.

    Main Methods:

    • Single-crystal X-ray diffraction was employed to determine the molecular and crystal structure.
    • Analysis of bond lengths, angles, and intermolecular contacts was performed.

    Main Results:

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    Characterizing Mammalian Zinc Transporters Using an In Vitro Zinc Transport Assay
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    Characterizing Mammalian Zinc Transporters Using an In Vitro Zinc Transport Assay

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    Thermochemical Studies of Ni(II) and Zn(II) Ternary Complexes Using Ion Mobility-Mass Spectrometry
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    Characterizing Mammalian Zinc Transporters Using an In Vitro Zinc Transport Assay
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    Characterizing Mammalian Zinc Transporters Using an In Vitro Zinc Transport Assay

    Published on: June 2, 2023

    • The crystal structure of [Zn(H(2)O)(6)](C(6)H(2)N(3)O(7))(2) was successfully determined.
    • The zinc(II) ion is octahedrally coordinated by six water molecules, residing on an inversion center.
    • Picrate anions do not exhibit direct coordination to the zinc(II) center; significant twisting of nitro groups from the benzene ring was observed.
    • Extensive intermolecular O-H⋯O hydrogen bonds were identified, contributing to the crystal packing.

    Conclusions:

    • The compound represents a hexaaquazinc(II) complex with picrate counterions.
    • The crystal structure is stabilized by a network of hydrogen bonds between coordinated water molecules and picrate anions.
    • The observed structural features provide insights into the supramolecular assembly of metal picrate complexes.